1. Qod: What two types of chemicals make up a chemical reaction?
Chemical Reactions
Qod:
What two types of chemicals make up a chemical reaction?

2. Chemical Reaction
A reaction in which one or more substances are changed to new substances
Reactants: ingredients needed to react
Products: new substances formed

3. No matter is created or destroyed
Law of Conservation
Total starting mass of all the reactants equals the total final mass of all products
No matter is created or destroyed

4. Symbols of Chemical Equation

5. Coefficients
The number of units of that element needed for the reaction
Subscripts
The number of atoms of that element

6. Balancing Chemical Reactions
Qod:
What would you do to remember the Six steps for Balancing Equations?

7. 6 Steps to Balancing Chemical Equations

8. 1. Write equation out to give you space

9. 2. Draw a line between reactants and products

10. 3. Write out each element present on each side
*Should be the same*

11. 4. Write the number of each element next to it

12. 5. Start with the left-most element and balance

13. 6. When finished with all elements on left side of equation, repeat steps 4 & 5 because you may have to redo some coefficients

14. Subscripts are used to balance charges
Coefficients are used to balance # of atoms
(Label your reactions with the following words: yields, products, reactants)

15. Examples
Ba P  Ba2 P3

16. K N  K3 N

17. Al CO3  Al CO3

18. Notebook Activity - #1

19. Notebook Activity - #2

20. Notebook Activity - #3

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22. Notebook Activity - #5

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24. Notebook Activity - #7

25. Notebook Activity - #8

27. Homework Problems

28. Homework Problems

29. Homework Problems

30. Homework Problems

31. Homework Problems

32. Homework Problems

33. Homework Problems

34. Homework Problems

35. Homework Problems

36. Homework Problems

37. 4 Types of Chemical Reactions
After today’s notes – make a chart or diagram on your left side that summarizes the four types of reactions

38. Combination(Synthesis) Reaction
Two reactants become one product!
Format: A X  AX
Ex #1: Na O H2O  Na OH
Ex #2: Ca S 

39. Decomposition Reaction
One reactant splits into two products
Format: AX  A + X
Ex #1:
Fe(OH)3  Fe OH

40. Single-Replacement Reaction
A single element swaps it mate from another
Format: A BX  B AX
Ex #1:
Al + H SO4  Al SO H

41. Ex #2: Fe + Cu2(SO4)3 

42. Double-Replacement Reaction
The elements are swapping!
Format: A+X- + B+Y-  A+Y- + B+X-
Ex #1:
Ba Cl + H SO4  Ba SO4 + HCl

43. Ex #2: H SO4 + Al OH 

44. Combustion Reaction Format: CXHY + O2  XCO2 + (Y/2)H2O
Oxygen reacts with a hydrocarbon to produce a carbon dioxide, water & energy (such as fire)
Format: CXHY + O2  XCO2 + (Y/2)H2O
Ex: C6H12O6 + O2 
Incomplete combustion produces CO (carbon monoxide) instead of CO2

45. Practice 1. ________ (NH4)3PO4 + BaCl  Ba PO4 + ___
Type Equation
1. ________ (NH4)3PO4 + BaCl  Ba PO ___
2. _________ Pb3P4 + Cl  _________ P
3. __________ KCO3  ______ ________
4. __________ Be + C2H3O2  __________

46. Affecting Reaction Rates
Temperature
Pressure
Substance Amounts

47. Reaction Rates Mole: amount of a substance
Catalyst: increases RR without being changed
End Result↓
Temperature
Surface Area
Concentration
Stirring
Reaction Rate ↑
Increase
Reaction Rate ↓
Decrease

48. https://www.youtube.com/watch?v=nsEkKIiOz7Q Reaction Lab